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WorksheetsChem 1010
Total questions: 97
Worksheet time: 8hrs 5mins
Name
Class
Date
1.
The reaction of 25 mL of N2 gas with 75 mL of H2 gas to form ammonia via the equation: N2 (g) + 3H2 (g) → 2NH3 (g)will produce ________ mL of ammonia if pressure and temperature are kept constant.
a)
100
b)
250
c)
150
d)
50
2.
The formula of nitrobenzene is C6H5NO2. The molecular weight of this compound is ________ g/mol.
a)
109.1
b)
3.06
c)
43.03
d)
123.11
3.
The mass % of C in methane (CH4) is ________.
a)
92.26
b)
133.6
c)
7.743
d)
74.87
4.
Calculate the percentage by mass of nitrogen in PtCl2(NH3)2.
a)
4.95
b)
9.9
c)
4.67
d)
9.34
5.
A 30.5 gram sample of glucose (C6H12O6) contains ________ mol of glucose.
a)
5.9
b)
0.169
c)
0.136
d)
0.424
6.
A nitrogen oxide is 63.65% by mass nitrogen. The molecular formula could be ________.
a)
NO2
b)
N2O4
c)
NO
d)
N2O
7.
There are ________ mol of carbon atoms in 4 mol of C4H8O2.
a)
20
b)
16
c)
8
d)
4
8.
There are ________ hydrogen atoms in 25 molecules of C4H4S2.
a)
25
b)
6.0 × 1025
c)
1.5 × 1025
d)
100
9.
What is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass?
a)
NaSO3
b)
Na2S2O6
c)
Na2S2O3
d)
NaSO
10.
A compound contains 40.0% C, 6.71% H, and 53.29% O by mass. The molecular weight of the compound is 60.05 g/mol. The molecular formula of this compound is ________.
a)
CH2O
b)
C2H4O2
c)
C2H3O4
d)
C2H2O4
11.
A compound that is composed of carbon, hydrogen, and oxygen contains 70.6% C, 5.9% H, and 23.5% O by mass. The molecular weight of the compound is 136 amu. What is the molecular formula?
a)
C5H6O2
b)
C8H4O
c)
C8H8O2
d)
C4H4O
12.
The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)When 2.5 mol of O2 are consumed in their reaction, ________ mol of CO2 are produced.
a)
3
b)
1.5
c)
2.5
d)
6
13.
Which combination will produce a precipitate?
a)
NaC2H3O2 (aq) and HCl (aq)
b)
KOH (aq) and Mg(NO3)2 (aq)
c)
NaOH (aq) and HCl (aq)
d)
NaF (aq) and HCl (aq)
14.
The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ________.
a)
SO42- (aq) + 2Na+ (aq) → 2Na+ (aq) + SO42-(aq)
b)
H+ (aq) + HSO4- (aq) + 2Na+ (aq) + 2OH- (aq) → 2H2O (l) + 2Na+ (aq) + SO42-(aq)
c)
H+ (aq) + OH- (aq) → H2O( l)
d)
H+ (aq) + HSO4- (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
15.
The reaction between strontium hydroxide and chloric acid produces ________.
a)
two molecular compounds
b)
two ionic compounds
c)
a molecular compound and an ionic compound
d)
an ionic compound
16.
In which reaction are electrons transfered from one species to another?
a)
HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
b)
2 AgNO3 (aq) + K2SO4 (aq) → 2 KNO3 (aq) + Ag2SO4 (s)
c)
2 Al(OH)3 (aq) + 3 H2SO4 (aq) → Al2(SO4)3 (s) + 6 H2O (l)
d)
2Na (s) + 2H2O (l) → 2NaOH (aq) + H2 (g)
17.
When the following reaction is balanced the coefficient in front of carbon dioxide is: ____ C5H12 + ____ O2 → ____ CO2 + ____ H2O
a)
6
b)
12
c)
10
d)
5
18.
When the following reaction is balanced the coefficient in front of oxygen is: ____ C8H18 + ____ O2 → ____ CO2 + ____ H2O
a)
12
b)
9
c)
25
d)
18
19.
In the correctly balanced reaction the coefficient for the H2O is: ____ Al(OH)3 + ____ H2SO4 → ____ Al2 (SO4)3 + ____ H2O
a)
1
b)
3
c)
6
d)
2
20.
When the reaction shown is balanced, there are ________ atoms of oxygen and ________ atoms of hydrogen on each side. (NH4)2SO4 (aq) + Ba(C2H3O2)2 (aq) → BaSO4 (s) + NH4C2H3O2 (aq)
a)
16; 28
b)
4; 7
c)
16; 18
d)
8; 14
21.
The dissolution of water in octane (C8H18) is prevented by ________.
a)
hydrogen bonding between water molecules
b)
dipole-dipole attraction between octane molecules
c)
hydrogen bonding between octane molecules
d)
ion-dipole attraction between water and octane molecules
22.
The principal reason for the extremely low solubility of NaCl in benzene (C6H6) is the ________.
a)
None
b)
hydrogen bonding in C6H6
c)
increased disorder due to mixing of solute and solvent
d)
weak solvation of Na+ and Cl- by C6H6
23.
Which one of the following substances is more likely to dissolve in benzene (C6H6)?
a)
CH3CH2OH
b)
CCl4
c)
NaCl
d)
HBr
24.
Which one of the following is most soluble in water?
a)
CH3CH2CH2OH
b)
CH3CH2CH2CH2CH2OH
c)
CH3CH2OH
d)
CH3OH
25.
Molarity is defined as the ________.
a)
moles solute/kg solution
b)
moles solute/kg solvent
c)
none (dimensionless)
d)
moles solute/liters solution
26.
The phrase "like dissolves like" refers to the fact that ________.
a)
polar solvents dissolve nonpolar solutes and vice versa
b)
gases can only dissolve other gases
c)
polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes
d)
condensed phases can only dissolve other condensed phases
27.
A solution with a concentration higher than the solubility is ________.
a)
unsaturated
b)
not possible
c)
supercritical
d)
supersaturated
28.
Which produces the greatest number of ions when one mole dissolves in water?
a)
glucose
b)
Na3PO4
c)
NaMnO4
d)
NH4Cl
29.
How many oxygen atoms are contained in 2.74 g of Al2(SO4)3?
a)
8.01 × 10-3
b)
12
c)
5.79 × 1022
d)
7.22 × 1024
30.
The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O:
C3H8 (g) + 5O2 (g) ? 3CO2 (g) + 4H2O (g)
When 2.5 mol of O2 are consumed in their reaction, ________ mol of CO2 are produced.
a)
1.5
b)
6
c)
3
d)
5
31.
The combustion of ammonia in the presence of oxygen yields NO2 and H2O:
4 NH3 (g) + 7 O2 (g) ? 4 NO2 (g) + 6 H2O (g)
The combustion of 43.9 g of ammonia with 258 g of oxygen produces ________ g of NO2.
a)
43.9
b)
212
c)
119
d)
0.954
32.
Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant:
2S (s) + 3O2 (g) ? 2SO3 (g)
In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. The % yield in this experiment is ________.
a)
29
b)
47
c)
88
d)
21
33.
How many grams of oxygen are in 56 g of C2H2O2?
a)
49
b)
19
c)
26
d)
31
34.
Lithium and nitrogen react to produce lithium nitride:
6Li (s) + N2 (g) ? 2Li3N (s)
How many moles of N2 are needed to react with 0.550 mol of lithium?
a)
3.3
b)
0.183
c)
0.0917
d)
0.55
35.
How many molecules are present in 4.25 mol of CCl4?
a)
2.56 × 1024
b)
36.91
c)
153.81
d)
9.26 × 1025
36.
Calculate the number of moles of aspirin, C9H8O4, in a 4.0 gram tablet.
a)
2.2 × 10-4
b)
0.022
c)
4.6 × 10-3
d)
2.2
37.
The number of grams in 0.350 mol of Na is ________.
a)
23
b)
0.35
c)
11
d)
8.05
38.
n the balanced reaction shown, the mole ratio of Fe2S3 to O2 is
Fe2S3 + 4 O2 ? 2 FeO + 3 SO2
a)
4 to 1.
b)
1 to 4.
c)
4 to 3.
d)
1 to 2.
39.
How many moles of CO2 are produced when 2.5 moles of O2 react according to the following equation?
C3H5 + 5 O2 ? 3 CO2 + 4 H2O
a)
1.5
b)
5
c)
18
d)
3
40.
The percentage yield of a reaction can best be described as the ________ times 100%.
a)
amount of desired product divided by the amount of unwanted product
b)
amount of product you could make if the reaction went to completion
c)
total amount of materials involved in a reaction
d)
amount of product obtained divided by the maximum possible amount of product
41.
The molar mass of Fe(OH)3 is ________ g/mole.
a)
89.87
b)
72.86
c)
106.87
d)
104.86
42.
Which of the following should be immiscible with carbon tetrachloride, CCl4?
a)
Br2
b)
CH3CH2OH
c)
C3H8
d)
C4H10
43.
What is the molarity of a solution prepared by dissolving 3.50 mol NaCl in enough water to make 1.50 L of solution?
a)
2.33 M
b)
137 M
c)
0.429 M
d)
87.8 M
44.
How many moles of HCl are present in 75.0 mL of a 0.200 M solution?
a)
0.375 mol
b)
0.0150 mol
c)
15.0 mol
d)
0.275 mol
45.
How many mL of 0.105 M AgNO3 are needed for an experiment that requires 0.00510 mol of AgNO3?
a)
17.8 mL
b)
18.70 mL
c)
20.6 mL
d)
48.6 mL
46.
How many g of CaCl2 are needed to prepare 500. mL of a 0.375 M solution?
a)
0.188 g
b)
20.8 g
c)
1.69 g
d)
3.00 g
47.
Which of the following has dispersion forces as its only intermolecular force?
a)
C6H13NH2
b)
CH4
c)
NaCl
d)
CH3Cl
48.
The predominant intermolecular force in NCl3 is ________.
a)
ion-dipole forces
b)
ionic bonding
c)
dipole-dipole forces
d)
London dispersion forces
49.
Of the following substances, only ________ has London dispersion forces as the only intermolecular force.
a)
NH3
b)
CH3OH
c)
Kr
d)
H2S
50.
The correct name for CCl4 is ________.
a)
carbon perchlorate
b)
carbon tetrachloride
c)
carbon tetrachlorate
d)
arbon chloride
51.
The correct name for N2O5 is ________.
a)
nitric oxide
b)
nitrogen oxide
c)
dinitrogen pentoxide
d)
nitrous oxide
52.
The molecular geometry of the PF3 molecule is ________, and this molecule is ________.
a)
trigonal pyramidal, nonpolar
b)
tetrahedral, unipolar
c)
trigonal planar, polar
d)
trigonal pyramidal, polar
53.
Of the following molecules, only ________ is polar.
a)
BeCl2
b)
NCl3
c)
BCl3
d)
Cl2
54.
The molecular geometry of the BrO3- ion is ________.
a)
tetrahedral
b)
T-shaped
c)
bent
d)
trigonal pyramidal
55.
The correct Roman numeral for the chromium ion in the compound CrCl3 is
a)
III
b)
I
c)
IV
d)
II
56.
Which of the following formulas in incorrect for a cobalt(III) compound?
a)
Co2O3
b)
CoCO3
c)
CoCl3
d)
CoPO4
57.
What is the formula of the nitrate ion?
a)
NO2 -1
b)
NO3 -1
c)
NO3 2-
d)
NO3 2-
58.
Which is the correct formula for the ionic compound containing iron(III) ions and oxide ions?
a)
Fe2O3
b)
FeO
c)
Fe3O2
d)
FeO2
59.
Which of the following is a molecular compound?
a)
RbBr
b)
CH3Cl
c)
CuCl2
d)
NaNO3
60.
Which of the following is an ionic compound?
a)
Mg3(PO4)2
b)
CH2O
c)
Cl2O
d)
PF5
61.
Determine the name for aqueous HBr.
a)
hydrobromic acid
b)
hydrogen bromate
c)
hydrobromous acid
d)
bromous acid
62.
Identify the formula for nitric acid.
a)
HNO2
b)
HNO4
c)
HNO3
d)
HNO
63.
The compound, ClO , is named
a)
chlorite.
b)
hypochlorite.
c)
chlorine (II) oxide.
d)
chlorine monoxide.
64.
The phosphorus atom in PCl3 would be expected to have a
a)
partial negative (?-) charge.
b)
partial positive (?+) charge.
c)
3+ charge.
d)
3- charge.
65.
In the Lewis structure of CH3OH, how many lone pairs of electrons are there?
a)
7
b)
3
c)
2
d)
5
66.
Place the following elements in order of decreasing electronegativity.
S Cl Se
a)
Cl > S > Se
b)
Se > Cl > S
c)
Se > S > Cl
d)
Cl > Se > S
67.
Choose the bond below that is most polar.
a)
C-C
b)
C-O
c)
C-F
d)
C-N
68.
Which molecule or compound below contains an ionic bond?
a)
C2Cl4
b)
OCl2
c)
NH4NO3
d)
SiF4
69.
Use the common ion charge to determine the chemical formula for the compound formed between Ca and N.
a)
CaN2
b)
Ca3N2
c)
Ca2N
d)
CaN
70.
The temperature of 25°C is __________ in Kelvins.
a)
166
b)
298
c)
248
d)
103
71.
The density of a gold nugget is 19.3 g/cm3. If the volume of the gold nugget is 0.00369 L, the mass of the nugget is ________ g.
a)
71.2
b)
5.23
c)
0.191
d)
19.3
72.
45 m/s = ________ km/hr
a)
1.6 × 102
b)
1.6 × 105
c)
0.045
d)
2.7
73.
The density of silver is 10.5 g/cm3. A piece of silver with a mass of 101 g would occupy a volume of ________ cm3.
a)
10.5
b)
9.62
c)
644
d)
0.171
74.
What happens to the mass number and the atomic number of an element when it undergoes beta (–) decay?
a)
The mass number decreases by 4 and the atomic number decreases by 2.
b)
The mass number does not change and the atomic number increases by 1.
c)
The mass number increases by 2 and the atomic number increases by 1.
d)
Neither the mass number nor the atomic number changes.
75.
All atoms of a given element have the same ________.
a)
number of neutrons
b)
number of protons
c)
number of electrons and neutrons
d)
density
76.
An atom of the most common isotope of gold, 197Au, has ________ protons, ________ neutrons, and ________ electrons.
a)
118, 79, 39
b)
197, 79, 118
c)
79, 118, 79
d)
79, 118, 118
77.
Isotopes are atoms that have the same ________ but differing ________.
a)
mass numbers, atomic numbers
b)
atomic numbers, mass numbers
c)
mass numbers, charges
d)
atomic masses, charges
78.
Elements ________ exhibit similar physical and chemical properties.
a)
in the same group of the periodic table
b)
with similar atomic masses
c)
with similar chemical symbols
d)
in the same period of the periodic table
79.
An element in the upper right corner of the periodic table ________.
a)
is definitely a nonmetal
b)
is either a metalloid or a nonmetal
c)
is either a metal or metalloid
d)
is definitely a metalloid
80.
Elements in Group 8A are known as the ________.
a)
alkaline earth metals
b)
noble gases
c)
alkali metals
d)
chalcogens
81.
Potassium is a ________ and chlorine is a ________.
a)
metalloid, nonmetal
b)
nonmetal, metal
c)
metal, nonmetal
d)
metal, metalloid
82.
The nucleus of an atom contains ________.
a)
protons
b)
electrons
c)
protons and electrons
d)
protons and neutrons
83.
Vertical columns of the periodic table are known as ________.
a)
groups
b)
metals
c)
periods
d)
metalloids
84.
How many total electrons are in the O2- ion?
a)
8
b)
18
c)
9
d)
10
85.
Which one of the following is a halogen?
a)
phosphorous
b)
argon
c)
sodium
d)
chlorine
86.
An atom of 118Xe contains ________ neutrons.
a)
172
b)
64
c)
110
d)
118
87.
Predict the charge of the most stable ion of aluminum.
a)
1+
b)
2+
c)
3-
d)
3+
88.
Which reaction is an example of an acid-base reaction?
a)
6 HCl(aq) + 2 Al(s) ? 2 AlCl3 (aq) + 3 H2 (g)
b)
H2SO4 (aq) + Ca(OH)2 (aq) ? CaSO4 (aq) + 2 H2O(l)
c)
2 Hg(l) + O2(g) ?2 HgO(s)
d)
FeCl3 (aq) + 3 KOH(aq) ? Fe(OH)3 (s) + 3 KCl(aq)
89.
2 AgNO3 (aq) + K2SO4 (aq) ? 2 KNO3 (aq) + Ag2SO4 (s)
The spectator ions in the reaction shown are
a)
potassium ion and nitrate ion.
b)
potassium ion and sulfate ion.
c)
silver ion and sulfate ion.
d)
silver ion and nitrate ion.
90.
All of the orbitals in a given electron shell have the same value as the ________ quantum number, n.
a)
psi
b)
magnetic
c)
spin
d)
principal
91.
There are ________ orbitals in the third shell.
a)
25
b)
1
c)
9
d)
16
92.
[Ar]4s23d104p3 is the electron configuration of a(n) ________ atom.
a)
V
b)
Sn
c)
P
d)
As
93.
The ground-state electron configuration of Sc is ________.
a)
1s22s22p63s23p63d3
b)
1s22s22p63s23p9
c)
1s22s22p63s23p64s23d1
d)
1s22s22p63s23p64s23d2
94.
An analysis showed a sample to contain 0.00471 grams of lead. How many micrograms is this?
a)
4.71 × 10-6 ?g
b)
4.71 × 10-2 ?g
c)
0.471 ?g
d)
4.71 × 103 ?g
95.
In scientific notation, the number 185,000,000 is
a)
1.85 × 106.
b)
1.85 × 108.
c)
1.85 × 10-8.
d)
185 × 106.
96.
How many significant figures are in the measurement, 0.0005890 g?
a)
7
b)
8
c)
5
d)
4
97.
An fossil specimen is found to be 65,200 years old. How many significant figures are there in this measurement?
a)
infinite
b)
four
c)
five
d)
three
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